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# 1- a) Write a net ionic equation for the neutralization of NaOH by a c.docx

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# 1- a) Write a net ionic equation for the neutralization of NaOH by a c.docx

1. a) Write a net ionic equation for the neutralization of NaOH by a component of a buffer buffer- .5M HC2H302/ .5M NaC2H302 (mixture of both) b) [then] Write a net ionic equaiton for the neutralization of HCL by a component of the buffer (addition of 3M HCI) c) compare your results in 2. and 3. Are the base-neutralizing capacity and the acid- neutralizing capacity of the buffer similar? Explain why or why not. 2. a) Write a net ionic equation for the neutralization of NaOH (3M) buffer .5M HC2H302 b) compare your results in 2 (above). and 5. Are the base-neutralizing capacities of bufer and acid comparable? Explain why or why not 3. a)Write a net ionic equation for the neutralization of HCL (3M) buffer .5M NaC2H302 b) compare your results in 3. and 6. Are the acid-neutralizing capacities of buffer and salt comparable? Explain why or why not.
Solution
1. Net ionic equation of buffer,
a) with NaOH
HC2H3O2(aq) + OH-(aq) --> C2H3O2-(aq) + H2O(l)
b) with HCl
C2H3O2-(aq) + H+(aq) --> HC2H3O2(aq)
2. with 3M NaOH,
it neutralizes the acid component of the buffer completely whose concentration in solution = 0.5 M HC2H3O2
3. with 3 M HCl, again the base component of the buffer is completely neutralized with added acid in solution. The concentration of base component of buffer is = 0.5 M.
Addition of excess base (NaOH) or acid (HCl) destroys the buffer and exceeds the buffer capacity. The solution is no more a buffer solution.
.

1. a) Write a net ionic equation for the neutralization of NaOH by a component of a buffer buffer- .5M HC2H302/ .5M NaC2H302 (mixture of both) b) [then] Write a net ionic equaiton for the neutralization of HCL by a component of the buffer (addition of 3M HCI) c) compare your results in 2. and 3. Are the base-neutralizing capacity and the acid- neutralizing capacity of the buffer similar? Explain why or why not. 2. a) Write a net ionic equation for the neutralization of NaOH (3M) buffer .5M HC2H302 b) compare your results in 2 (above). and 5. Are the base-neutralizing capacities of bufer and acid comparable? Explain why or why not 3. a)Write a net ionic equation for the neutralization of HCL (3M) buffer .5M NaC2H302 b) compare your results in 3. and 6. Are the acid-neutralizing capacities of buffer and salt comparable? Explain why or why not.
Solution
1. Net ionic equation of buffer,
a) with NaOH
HC2H3O2(aq) + OH-(aq) --> C2H3O2-(aq) + H2O(l)
b) with HCl
C2H3O2-(aq) + H+(aq) --> HC2H3O2(aq)
2. with 3M NaOH,
it neutralizes the acid component of the buffer completely whose concentration in solution = 0.5 M HC2H3O2
3. with 3 M HCl, again the base component of the buffer is completely neutralized with added acid in solution. The concentration of base component of buffer is = 0.5 M.
Addition of excess base (NaOH) or acid (HCl) destroys the buffer and exceeds the buffer capacity. The solution is no more a buffer solution.
.

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### 1- a) Write a net ionic equation for the neutralization of NaOH by a c.docx

1. 1. 1. a) Write a net ionic equation for the neutralization of NaOH by a component of a buffer buffer- .5M HC2H302/ .5M NaC2H302 (mixture of both) b) [then] Write a net ionic equaiton for the neutralization of HCL by a component of the buffer (addition of 3M HCI) c) compare your results in 2. and 3. Are the base-neutralizing capacity and the acid- neutralizing capacity of the buffer similar? Explain why or why not. 2. a) Write a net ionic equation for the neutralization of NaOH (3M) buffer .5M HC2H302 b) compare your results in 2 (above). and 5. Are the base- neutralizing capacities of bufer and acid comparable? Explain why or why not 3. a)Write a net ionic equation for the neutralization of HCL (3M) buffer .5M NaC2H302 b) compare your results in 3. and 6. Are the acid-neutralizing capacities of buffer and salt comparable? Explain why or why not. Solution 1. Net ionic equation of buffer, a) with NaOH HC2H3O2(aq) + OH-(aq) --> C2H3O2-(aq) + H2O(l) b) with HCl C2H3O2-(aq) + H+(aq) --> HC2H3O2(aq) 2. with 3M NaOH, it neutralizes the acid component of the buffer completely whose concentration in solution = 0.5 M HC2H3O2 3. with 3 M HCl, again the base component of the buffer is completely neutralized with added acid in solution. The concentration of base component of buffer is = 0.5 M. Addition of excess base (NaOH) or acid (HCl) destroys the buffer and exceeds the buffer capacity. The solution is no more a buffer solution.